<p>I know this is easy, but i have missed class all week and am.. confused</p>
<p>How many moles of solute are contained in 500 g of a 2.00% aqueous solution of K2Cr2O7</p>
<p>I am no chemistry expert, but since its 2% solvent, I would think that it would be 98% solute.</p>
<p>So 490 g of solute are present. Next find the molecular weight of K2Cr2O7 and convert to moles. Do 490/molar weight of compound.</p>
<p>(This is just a guess)</p>
<p>I would have thought that it would mean 2% of the compound, and 98% water. (I'm not sure though, so don't quote me on it. I'll try to confirm which one it is)</p>
<p>Either way, you'd divide the weight of the solute, by the molar mass of the compound, to get moles.</p>
<p>yeah.. i knew that you divided it by the molar mass but wasnt sure what the 2 % represented</p>
<p>if it's 2%, then::</p>
<p>.02 x 500 = 10 grams solution
490 grams K2Cr2O7</p>
<p>so...</p>
<p>(490 grams / molar mass of K2Cr2O7) = number of moles</p>
<p>It would be 2% K2Cr2O7 (solute) and 98% H2O (solvent)</p>
<p>So 0.02X500 = 10g Solute = 10g K2Cr2O7</p>
<p>10g/molar mass of K2Cr2O7 = mole</p>
<p>Note: I asked my parents, and they told me that the 2% refers to the solute, in this case, K2Cr2O7.</p>
<p>Thank you!</p>